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chemistry (ct version) > mdm. everything > Flashcards

mdm. everything Flashcards

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1
Q

what determines the electric field behaviour

A
  1. direction of deflection (charge)
  2. angle of deflection
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2
Q

what is the angle of deflection changed by

A
  • the magnitude of particle: determined by charge and mass
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3
Q

what are the three laws to explain electronic configurations

A
  1. Aufbom (4s>3d)
  2. Hund’s ( minimise inter-electronic repulsion)
  3. Pauli Exclusion
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4
Q

what did the pauli exclusion theory explain

A

2 electrons of opposite spins will counterbalance the electrical repulsion (from identical charges)

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5
Q

what affects the electrostatic effects

A
  • number of electronic shells
  • nuclear charge
  • shielding effect
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6
Q

what does electronegativity depend on

A

the electrostatic forces of attraction between the nucleus and valence electrons

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7
Q

what does the ionic bond strength depend on

A
  • charge (from electrostatic attraction)
  • radius/size (inter-ionic dist)
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8
Q

what determines the strength of metallic bonds

A
  • number of valence electrons available
  • cation charges
  • cation sizes
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9
Q

what is the bond angle affeted by

A

electronegativity and number of lone pair electrons

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10
Q

describe idid moments

A

momentary movements of electrons in particles will cause the electron density to be unsymmetrical: instantaneous dipole will induce a dipole on neighbouring particles, which attraction is short-lived as the electrons keep moving and the dipoles vanish and reform

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11
Q

what affects idid

A
  • number of electrons/electron cloud size (size and ease of polarisability)
  • surface area for molecular interaction (straight chains>branched)
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12
Q

what is hydrogen bonding

A

the highly electronegative hydrogen atom can form a particularly strong attraction with lone pair electrons on adjacent molecules and the intermolecular FOA= hydrogen bonding

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13
Q

what is covalent bond strength

A

average energy required to break one mole of a particular bond in gaseous state

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14
Q

what affects the covalent bond strength

A
  • effectiveness of overlap
  • number of bonds between the atom
  • bond polarity
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15
Q

what are the effects of hydrogen bonding (IMFOA)

A
  • explain diff in b.p of grp 4, 5, 6
  • b.p of NH3 and HF
  • open structure of ice
  • dimerisation of carboxylic acids
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16
Q

carboxylic acids are dimers in

A
  • vapour state
  • non-polar solvents
17
Q

what determines the degree of covalence

A
  • cation’s polarising power
  • anion’s polarising power
18
Q

what affects the solubility

A
  • strength of bond
  • extensiveness of hydrogen bonding
19
Q

what are the three gaseous laws

A
  • avogradro’s law
  • gay-lussac’s law ( pressure and temp)
  • charles (vol. and temp)
  • bolyes’ (volxpressure=vol. pa)
20
Q

what is 1atm and 1 bar equivalent to

A

101325 Pa and 10^6 Pa

21
Q

what does the kinetic theory of gases state

A
  • particles of negligible volume
  • particles of negligible attractive forces
  • in constant random motion
  • perfectly elastic collisions
  • avg KE directly proportional to absolute temp
22
Q

2 conditions real gases become more ideal

A
  • higher temp (overcome IMF=negligible)
  • lower pressure (particles’ volume become negligible compared to container’s volume)
23
Q

why are gases not ideal

A

particles have a finite volume and size; the presence of attractive forces between gas particles

24
Q

what determines the extent of positive and negative deviations

A
  • bondings btwn (strong/weak idid/ pdpd/H bonding)
  • larger electron cloud size (stronger intermolecular attractions and more easily POLARISED)
25
Q

units of ideal gas equation

A

pV=nRT
*p=Pa
*V=m^3
*T=Kelvin

26
Q

factors affecting lattice energy

A
  • effect of ionic charge (bigger cation/anionic charge–> greater MAGNITUDE)
  • effect of ionic size (smaller=larger magnitude)
27
Q

assumptions made during experimental

A
  • density of solution=density of water
  • specific heat capacity refers to water’s
  • heat loss to surroundings CORRECTED by extrapolation

chemistry (ct version) (3 decks)

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